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This leads to protonation of very strong acids like hydrochloric, sulfuric, or nitric acids when using concentrated hydrofluoric acid solutions. [21] Although hydrofluoric acid is regarded as a weak acid, it is very corrosive, even attacking glass when hydrated. [20] Dilute solutions are weakly acidic with an acid ionization constant K a = 6.6 ...
Aqueous solutions of HF are called hydrofluoric acid. When dilute, hydrofluoric acid behaves like a weak acid, unlike the other hydrohalic acids, due to the formation of hydrogen-bonded ion pairs [H 3 O + ·F −]. However concentrated solutions are strong acids, because bifluoride anions are predominant, instead
Hydrofluoric acid is a weak acid in aqueous solution (pK a = 3.15) [7] but a very weak acid in the gas phase (E pa (F −) = 1554 kJ/mol): [4] the fluoride ion is as strong a base as SiH 3 − in the gas phase, but its basicity is reduced in aqueous solution because it is strongly hydrated, and therefore stabilized.
Hydrogen fluoride, a weak acid in aqueous solution that is normally not thought to have any appreciable Brønsted basicity at all, is in fact the strongest Brønsted base in the mixture, protonating to H 2 F + in the same way water protonates to H 3 O + in aqueous acid. It is the fluoronium ion that accounts for fluoroantimonic acid's extreme ...
For example, acetic acid is a weak acid which has a = 1.75 x 10 −5. Its conjugate base is the acetate ion with K b = 10 −14 /K a = 5.7 x 10 −10 (from the relationship K a × K b = 10 −14), which certainly does not correspond to a strong base. The conjugate of a weak acid is often a weak base and vice versa.
The biggest concern is that the refinery continues to use the highly toxic chemical hydrofluoric acid to process fuel, a practice that Schwartz and other activists want to see stopped.
Unlike other hydrohalic acids, such as hydrochloric acid, hydrogen fluoride is only a weak acid in water solution, with acid dissociation constant (pK a) equal to 3.19. [36] HF's weakness as an aqueous acid is paradoxical considering how polar the HF bond is, much more so than the bond in HCl, HBr, or HI. The explanation for the behavior is ...
All of these compounds form acids when mixed with water. Hydrogen fluoride is the only hydrogen halide that forms hydrogen bonds. Hydrochloric acid, hydrobromic acid, hydroiodic acid, and hydroastatic acid are all strong acids, but hydrofluoric acid is a weak acid. [16] All of the hydrogen halides are irritants.